Assertion : In the proces, `H_(2(g)) rarr 2H_((g))`.entropy increases.
Reason : Breaking of bonds is an endothermic process.

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion.
B. If both assertion and reason are true but reason is not the correct explanation of assertion
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question, we need to analyze both the assertion and the reason provided.

### Step 1: Analyze the Assertion
The assertion states that in the process \( H_2(g) \rightarrow 2H(g) \), entropy increases.
- **Explanation**: Entropy is a measure of disorder in a system. In this reaction, one molecule of diatomic hydrogen gas (\( H_2 \)) is converted into two separate hydrogen atoms (\( 2H \)).
- Since there is an increase in the number of gas particles from 1 to 2, the system becomes more disordered. Therefore, the entropy of the system increases.

### Step 2: Analyze the Reason
The reason states that breaking of bonds is an endothermic process.
- **Explanation**: Breaking chemical bonds requires energy, which is supplied in the form of heat. This process is indeed endothermic because energy is absorbed to break the bonds between the atoms in \( H_2 \).

### Step 3: Determine the Relationship
Now, we need to determine if the reason correctly explains the assertion.
- While it is true that the breaking of bonds is an endothermic process, this does not directly explain why the entropy increases in the reaction. The increase in entropy is due to the increase in the number of gaseous particles, not solely because the process is endothermic.

### Conclusion
- Both the assertion and the reason are true.
- However, the reason does not provide a correct explanation for the assertion.

Thus, the final answer is: **Option 2: Both assertion and reason are true, but the reason is not the correct explanation of the assertion.**

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